Chemistry Mole and Quantum Concepts
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Questions and Answers

How many orbitals are found in the d subshell?

  • 7
  • 3
  • 1
  • 5 (correct)

What does an increase in ionization energy as we move across a period indicate?

  • Decrease in nuclear charge
  • Increase in atomic size
  • Decrease in electron-electron repulsion
  • Increase in effective nuclear charge (correct)

Why does the first ionization energy decrease as we go down Group 1?

  • Increased electron-electron repulsion
  • Increased distance between nucleus and electrons (correct)
  • Decreased nuclear charge
  • Decreased number of energy shells

Which block in the periodic table typically contains the elements with the highest ionization energies?

<p>p block (B)</p> Signup and view all the answers

What is the trend of atomic radius as you move down a group in the periodic table?

<p>It increases (D)</p> Signup and view all the answers

What does a large jump in ionization energies indicate about the configuration of an atom?

<p>Removal of an electron from a filled subshell (B)</p> Signup and view all the answers

How many electrons can be held in the f subshell?

<p>14 (C)</p> Signup and view all the answers

Which group does not follow the expected trend of increasing ionization energy across the period?

<p>Group 3 (B)</p> Signup and view all the answers

What defines an electrophile in a chemical reaction?

<p>A species that accepts electrons (C)</p> Signup and view all the answers

Which of the following correctly describes the major product formed from electrophilic addition involving a tertiary carbocation?

<p>It is typically more stable than the minor product (C)</p> Signup and view all the answers

What is the key consequence of incineration of non-biodegradable polymers?

<p>Increase in greenhouse gas emissions (C)</p> Signup and view all the answers

How would you convert between addition polymerisation and monomers?

<p>By applying changes in temperature and pressure (C)</p> Signup and view all the answers

Which of the following statements about biodegradable polymers is correct?

<p>They can reduce environmental pollution when disposed of correctly (C)</p> Signup and view all the answers

What is a defining property of homolytic fission in a chemical reaction?

<p>Two free radicals with unpaired electrons are generated (A)</p> Signup and view all the answers

What is the primary problem associated with the production of non-biodegradable polymers?

<p>They contribute to long-term pollution and landfill overflow (A)</p> Signup and view all the answers

What is the result of incomplete combustion of organic compounds?

<p>Creation of toxic by-products such as carbon monoxide (B)</p> Signup and view all the answers

Which type of reaction involves the exchange of atoms or groups between molecules?

<p>Substitution Reaction (A)</p> Signup and view all the answers

What is the primary purpose of fractional distillation in the processing of crude oil?

<p>To separate substances based on boiling points (A)</p> Signup and view all the answers

Which type of bond fission involves the equal splitting of electrons?

<p>Homolytic Fission (A)</p> Signup and view all the answers

What are the potential environmental consequences of oxides of nitrogen emissions?

<p>Acid rain formation (C)</p> Signup and view all the answers

Which process converts straight-chain organic compounds into branched-chain compounds?

<p>Reforming (C)</p> Signup and view all the answers

Which type of combustion results in the production of carbon monoxide and other pollutants?

<p>Incomplete Combustion (A)</p> Signup and view all the answers

What is the significance of carbon neutrality?

<p>Balancing emitted carbon with carbon offsetting (D)</p> Signup and view all the answers

What distinguishes biofuels from natural gas in terms of sustainability?

<p>Biofuels are renewable and can be produced sustainably (A)</p> Signup and view all the answers

What type of overlap leads to the formation of sigma bonds?

<p>End on overlap of atomic orbitals (A)</p> Signup and view all the answers

What is the relationship between bond length and bond strength?

<p>As bond length decreases, bond strength increases (C)</p> Signup and view all the answers

How does electronegativity change across a period in the periodic table?

<p>It increases (D)</p> Signup and view all the answers

Which statement about pi bonds is correct?

<p>They exist only in double or triple bonded atoms (C)</p> Signup and view all the answers

What characterizes a dative covalent bond?

<p>One atom provides both electrons for the bond (B)</p> Signup and view all the answers

In what state can ionic compounds conduct electricity?

<p>Only when dissolved in water or in molten state (B)</p> Signup and view all the answers

What is the primary cause of electronegativity in atoms?

<p>The number of protons in the nucleus (D)</p> Signup and view all the answers

Which of the following correctly represents the trend of electronegativity down a group in the periodic table?

<p>Electronegativity decreases down a group (B)</p> Signup and view all the answers

Which type of formula explicitly shows every atom and bond in a molecule?

<p>Displayed formula (B)</p> Signup and view all the answers

What is the term for the simplest whole number ratio of a molecular formula?

<p>Empirical formula (D)</p> Signup and view all the answers

Which type of isomer is defined as having different carbon chains?

<p>Chain isomers (B)</p> Signup and view all the answers

What defines electrophiles in chemical reactions?

<p>They are attracted to regions of high electron density. (A)</p> Signup and view all the answers

Which process breaks down long-chained molecules into shorter chains?

<p>Cracking (B)</p> Signup and view all the answers

In structural isomers, what characteristic do the compounds share?

<p>Same molecular formula, different structures (D)</p> Signup and view all the answers

What characterizes the major product in addition reactions involving carbocations?

<p>It results from a secondary carbocation due to stability. (D)</p> Signup and view all the answers

In the electrophilic addition of halogens, what causes the halogen molecule to become polar?

<p>The repulsion of the bonding electrons by the pi-bond's electron cloud. (C)</p> Signup and view all the answers

What is the outcome when heterolytic fission occurs in a covalent bond?

<p>A single atom takes both bonding electrons. (D)</p> Signup and view all the answers

Which reaction involves two reactants combining to form a single product?

<p>Addition reaction (D)</p> Signup and view all the answers

What is defined as a repeat unit in polymer chemistry?

<p>The set of atoms that join together to form a polymer. (B)</p> Signup and view all the answers

Which of the following statements is true regarding traditional plastic waste?

<p>It is non-biodegradable and can produce harmful emissions when burned. (B)</p> Signup and view all the answers

What is a key factor that allows alkenes to have geometric isomers?

<p>The existence of at least one double bond in the compound. (C)</p> Signup and view all the answers

What must be present for a compound to exhibit geometric isomerism?

<p>Different substituents on each side of a double bond. (D)</p> Signup and view all the answers

Which condition must not be present for alkanes to exhibit geometric isomerism?

<p>The presence of double bonds. (A)</p> Signup and view all the answers

What is the outcome of addition polymerization involving alkenes?

<p>The formation of a polymer by breaking alkene double bonds. (C)</p> Signup and view all the answers

Flashcards

Ionisation Energy

The energy required to remove one electron from a neutral gaseous atom in its ground state.

Reactivity

The tendency of an element to lose an electron.

Atomic Radius

The distance between the nucleus and the outermost electron shell in an atom.

Second Ionisation Energy

The energy required to remove the second electron from a unipositively charged gaseous ion in its ground state.

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Third Ionisation Energy

The energy required to remove the third electron from a dipositively charged gaseous ion in its ground state.

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Ionisation Energy Trend (Across Period)

The general trend of increasing ionisation energy as you move from left to right across a period in the periodic table.

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Ionisation Energy Trend (Down Group)

The general trend of decreasing ionisation energy as you move down a group in the periodic table.

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Big Jumps in Ionisation Energies

The sharp increases in successive ionisation energies indicate the removal of an electron from a stable, complete electron shell.

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Ionic Compounds and Electrical Conductivity

Ionic compounds conduct electricity when dissolved in water or in a molten state. This happens because the ions become mobile and can migrate towards electrodes with opposite charges when a potential difference is applied.

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Covalent Bond Formation

A covalent bond forms when two atoms share a pair of electrons. This sharing occurs when atomic orbitals containing single electrons from each atom overlap.

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Sigma Bonds

An overlap of atomic orbitals along the internuclear axis forms a sigma bond. It results in a strong and stable bond.

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Pi Bonds

A sideways overlap of p orbitals forms a pi bond. This bond is weaker than a sigma bond and only forms after a sigma bond is established.

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Pi vs Sigma Bond Strength

Pi bonds are weaker than sigma bonds because the electron density is located above and below the internuclear axis, resulting in less effective overlap.

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Bond Length and Strength

Bond length measures the distance between the nuclei of two covalently bonded atoms. As bond length decreases, the bond strength increases due to stronger electrostatic attraction between the nuclei and shared electrons.

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Electronegativity

Electronegativity is an atom's ability to attract a bonding pair of electrons towards itself. Atoms with higher electronegativity values attract electrons more strongly.

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Electronegativity Trends

Electronegativity increases across a period due to increasing nuclear charge, pulling electrons closer. Down a group, electronegativity decreases due to increased atomic size and shielding effect, weakening the attraction.

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Saturated

A compound containing only single bonds.

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Unsaturated

A compound containing one or more double bonds.

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Displayed Formula

Shows every atom and every bond in a molecule.

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Structural Formula

Shows how the atoms are joined together in a molecule, but not necessarily the exact positions of atoms.

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Skeletal Formula

Shows all the bonds between carbon atoms, but not the hydrogen atoms.

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Molecular Formula

Shows the count of each atom in a molecule.

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Empirical Formula

The simplest whole number ratio of the molecular formula.

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Functional Group

An atom or group of atoms in a molecule that’s responsible for its chemical reactions.

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Positional Isomers

Isomers that differ in the position of a functional group on the carbon chain.

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Addition Reaction

A type of chemical reaction where two or more molecules combine to form a larger molecule.

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Substitution Reaction

A type of chemical reaction where an atom or group of atoms in a molecule is replaced by another atom or group of atoms.

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Homolytic Fission

A process that involves the breaking of a covalent bond where each of the bonded atoms receives one electron from the shared pair.

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Crude Oil

The natural mixture of hydrocarbons found in the Earth's crust.

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Fractional Distillation

A process that separates crude oil into different fractions based on their boiling points.

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Cracking

A process that breaks down large hydrocarbon molecules into smaller, more useful ones.

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Reforming

A process that converts straight-chain alkanes into branched alkanes or aromatic hydrocarbons.

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Addition Polymerization

The formation of a polymer by the addition of monomers to an existing polymer chain, resulting in a long chain of repeating units. No small molecules are released during the reaction.

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Alkene

A molecule containing a carbon-carbon double bond.

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Polymer

A compound formed by the combination of two or more molecules of the same type (monomers).

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Monomer

A small molecule that can combine with other identical molecules to form a larger molecule (polymer).

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Repeat unit

A repeating unit within a polymer structure. Represents the basic structure that is repeated multiple times.

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Geometric isomer

An isomer that has the same atoms connected in the same order but differs in the spatial arrangement of the atoms around the double bond. They can be cis/Z or trans/E.

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Carbocation stability

Stability of carbocations in a reaction increases with the number of alkyl groups attached to the positively charged carbon atom. Tertiary carbocations are most stable, followed by secondary, and primary carbocations are least stable.

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Electrophilic Addition

A reaction where an electrophile, an electron-seeking species, attacks a double or triple bond in an alkene or alkyne, leading to the formation of a new single bond.

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Electrophile

A species deficient in electrons, having a positive charge or a partially positive charge, seeking electrons to form a bond.

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Electrophilic Addition: Hydrogen Halides

In this type of reaction, a hydrogen halide (HX) molecule adds across a carbon-carbon double bond. The hydrogen atom adds to the carbon atom that already has more hydrogen atoms (Markovnikov's rule).

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Electrophilic Addition: Halogens

In this type of reaction, a halogen molecule (X2) adds across a carbon-carbon double bond. The two halogen atoms add to the same carbon, forming a dihaloalkane.

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Major & Minor Products: Carbocation Stability

In electrophilic addition, the formation of carbocations can lead to 'major' or 'minor' products, depending on the stability of the carbocations. Tertiary carbocations are the most stable, followed by secondary, and then primary carbocations.

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Non-Biodegradable Polymers

Polymers that cannot be broken down by microorganisms, persisting in the environment for long periods, causing pollution.

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Biodegradable Polymers

Polymers that can be broken down by microorganisms into simpler substances, reducing environmental impact.

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Study Notes

Topic 1 Check List

  • Avogadro's Constant definition is required.
  • Mole definition is required.
  • Mole calculations include molecules, atoms, ions, protons, neutrons, and electrons.
  • Mole rules: n = m/Mr, n = CV, n = V/24
  • Mole Ratio usage is needed.
  • Molar Ratios for excess reactants and gas volumes.
  • Percentage yield and percentage purity formula.
  • Atom economy formula.
  • Empirical formula calculations.
  • Molecular formula from empirical formula calculations.
  • Water of crystallisation calculations using molar ratio rule & Mr of whole hydrated crystals.
  • Ideal gas rules and SI measurements.
  • Converting Celsius to Kelvin is needed.
  • Molar concentration versus mass concentration differences.
  • Definition of Parts per million (PPM).
  • PPM rule is required.

Topic 2 Check List

  • Sub-atomic particle masses and charges.
  • Quantum shells, sub-shells, and orbitals.
  • Energy trends between sub-shells and quantum shells.
  • Number of sub-shells and their shape (S & P orbitals).
  • Electron capacity of orbitals and sub-shells.
  • Electron arrangement order in sub-shells.
  • Electronic configurations for elements.
  • Electron removal order from sub-shells.
  • Periodic table block positions (s, p, d, f).
  • Periodic table group assignments.
  • Electronic configuration of 24Cr and 29Cu.
  • Ionisation energy definition.
  • Trends in ionisation energy (group and period).
  • Trend in first ionisation energy in group 1.
  • Relationship between reactivity and ionisation energy.
  • Significance of large jumps in ionisation energies.
  • Reasons for successive ionisation energy increases.

Topic 3 Check List

  • Ionic bonding definition.
  • Ionic bonding establishment.
  • Factors affecting ionic bond strengths (ion sizes and charges).
  • Evidence for ions' existence (electrolysis and electron density maps).
  • Ionic radii trends (group and period).
  • Polarisation and polarising power definitions.
  • Factors affecting polarisation (ion sizes and charges).
  • Covalent character in ionic compounds.
  • Ionic compound properties (melting/boiling points, water solubility, electrical conductivity, brittleness).
  • Covalent bonding definition.
  • Covalent bond formation (orbital overlapping).

Topic 4 Check List

  • Hydrocarbon definition.
  • Saturated vs. unsaturated compounds.
  • Formula types (general, molecular, empirical, displayed, structural, skeletal).
  • Functional group definition.
  • Homologous series definition and properties.
  • Naming compounds using prefixes and suffixes.
  • Isomerism definition and types (chain, functional group, positional).
  • Isomerism in alkanes (2n-4+1).
  • Cycloalkanes vs. alkanes.
  • Addition reaction types.
  • Bond breaking types (homolytic and heterolytic fission).
  • Alkyl group structure and general formulas.
  • Crude oil processes (fractional distillation, cracking, reforming).
  • Properties of organic compounds used in fractional distillation.
  • Upper/lower molecule properties in fractional distillation columns (boiling point, colour, etc).
  • Cracking products and conditions.
  • Reforming of straight-chain compounds, and conditions
  • . Complete vs. incomplete combustion.
  • Combustion emission problems.

Topic 5 Check List

  • Unsaturated hydrocarbon definition.
  • Alkene general formula.
  • Cycloalkane general formula.
  • Sigma and pi bond types in double bonds.
  • Drawing sigma and pi bonds in double bonds.
  • Stereoisomers/Geometric isomers.
  • Conditions for geometric isomerism.
  • Alkane geometric isomerism inability.
  • Number of geometric isomers for a double bond.
  • Trans/Cis/E/Z designations in alkenes.
  • Electrophilic addition reaction definitions and types.
  • Electrophilic addition mechanism for hydrogen halides and halogens.
  • Major/minor products formation in electrophilic addition mechanisms (primary/secondary/tertiary carbocations).
  • Addition polymerization and monomers.
  • Definition of electrophilic addition.
  • Electrophile definition.
  • Conversion between addition polymerizations and monomers
  • Non-biodegradable vs. biodegradable polymers.
  • Polymer waste management (incineration).

Essential Equations

  • First and second ionisation energy equations.
  • Mass spectrometry, homolytic/heterolytic fission equations, with conditions.

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Description

Test your understanding of essential chemistry concepts, including the definitions and calculations of moles, Avogadro's constant, and different particle definitions. Additionally, assess your knowledge of quantum mechanics, energy levels, and sub-atomic particles. This quiz covers both foundational mole concepts and advanced quantum shell configurations.

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